Question

methane gas and chlorine gas react to form hydrogen chloride gas and carbon tetrachloride gas. what volume of hydrogen chloride would be produced by this reaction if 7.0 ml of methane were consumed? also, be sure your answer has a unit symbol, and is rounded to 2 significant digits.

Explanation:

Step1: Write the balanced reaction

The reaction between methane ($\ce{CH4}$) and chlorine ($\ce{Cl2}$) to form carbon tetrachloride ($\ce{CCl4}$) and hydrogen chloride ($\ce{HCl}$) is:
$$\ce{CH4 + 4Cl2 -> CCl4 + 4HCl}$$

Step2: Determine the mole ratio

From the balanced equation, 1 mole of $\ce{CH4}$ produces 4 moles of $\ce{HCl}$. For gases at the same temperature and pressure, volume ratios are equal to mole ratios (Avogadro's law). Thus, the volume ratio of $\ce{CH4}$ to $\ce{HCl}$ is $1:4$.

Step3: Calculate the volume of $\ce{HCl}$

Given volume of $\ce{CH4}$ = $7.0\ \text{mL}$. Let $V_{\ce{HCl}}$ be the volume of $\ce{HCl}$.
Using the ratio:
$$V_{\ce{HCl}} = 4 \times V_{\ce{CH4}}$$
$$V_{\ce{HCl}} = 4 \times 7.0\ \text{mL}$$
$$V_{\ce{HCl}} = 28\ \text{mL}$$ (rounded to 2 significant digits)

Answer:

$28\ \text{mL}$